Friday
April 18, 2014

Search: Calculate the pH of 0.10 M aqueous solution of each of the hydrochloric and acetic acids: Complete the following table.

Number of results: 110,766

chemistry
What is the original molarity of an aqueous solution of ammonia (NH3) whose pH is 11.10 at 25 degrees C? (Kb for NH3=1.8 x 10^-5)
Wednesday, December 8, 2010 at 4:44pm by Natalie

Chemistry
What is the PH of a buffer made by adding 8.20 grams of sodium acetate(NaCH3CO2) to 500 ml of 0.10 M acetic acid(CH3CO2H). Ka for acetic acid is 1.8 x 10^-5.
Sunday, April 14, 2013 at 8:17pm by Lele

university of the west indies
The pH of a 0.164 M aqueous solution of dimethylamine is 11.98. Write the ionization equation, calculate the values of Kb and pKb and comment on strength of the base....
Wednesday, September 19, 2012 at 10:10pm by geeta

Chemistry
A beaker with 150 mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 5.60 mL of a 0.280 M HCl solution to the beaker. How much will the pH change? The pKa of acetic ...
Thursday, July 9, 2009 at 2:01am by Saira

chemistry help!!
A beaker with 195 mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 8.20 mL of a 0.260 it M HCl solution to the beaker. How much will the pH change? The pKa of acetic ...
Monday, July 13, 2009 at 1:10pm by DrFunk

Chemistry
A beaker with 150 mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 7.90 mL of a 0.480 M HCl solution to the beaker. How much will the pH change? The pKa of acetic ...
Tuesday, October 6, 2009 at 8:06pm by Anonymous

Chemistry
What would be the pH of a 0.1 M aqueous solution of the phenolate ion, C6H5O–? (Ka for phenol, C6H5OH, is 1.3 x 10–10) I got the answer 5.44 but I think it's wrong. Do I have to subtract it from 14?
Saturday, July 6, 2013 at 12:38am by Nat

chemistry
What should be the pH of the aqueous layer to extract caffeine? There are three aqueous solutions that you may choose from. Answer A. pH >14, using 2.5 M NaOH (aq) B. pH 1, using 0.1 M HCl (aq) C. pH 6.2, using 0.1 M NaHCO3 (aq)
Thursday, May 30, 2013 at 9:41am by A

chemistry
What should be the pH of the aqueous layer to extract caffeine? There are three aqueous solutions that you may choose from. Answer A. pH >14, using 2.5 M NaOH (aq) B. pH 1, using 0.1 M HCl (aq) C. pH 6.2, using 0.1 M NaHCO3 (aq)
Thursday, May 30, 2013 at 6:04pm by A

chemistry
The pKa for hydrochloric acid is −6.0. What is the concentration of HCl(aq) we would expect to find in a 1 M solution of hydrochloric acid? What pH would we expect? how do you solve this problem?
Tuesday, July 6, 2010 at 11:31pm by Jin

Chemistry
0.15g of hydrogen chloride HCl is dissolved in water to make 8.0L of solution. What is the pH of the resulting hydrochloric acid solution?
Friday, March 1, 2013 at 10:46am by Jonah

CHEMISTRY
0.15g of hydrogen chloride (HCl) is dissolved in water to make 6.5L of solution. What is the pH of the resulting hydrochloric acid solution?
Monday, February 17, 2014 at 11:21pm by Anonymous

Chemistry
Find the pH: 1) A 0.001M solution of HCl 2) A 7.98 x 10^-2 M solution of HNO3 3) 1098L of a solution containing 8.543moles of HBr 4) 120mL of a solution containing 0.005 grams of hydrochloric acid. Please help me with these four. Out of 20 questions i only didn't understand ...
Wednesday, March 20, 2013 at 7:01pm by Katelyn

chem
a buffer is made by adding 150 ml of .595M BaF2 and 0f .500M of HF solution. calculate the pH of this buffer system calculate the pH of this buffer after adding .100 mol Hcl calculate the pH of this buffer after adding .0750 mol Ca(OH)2 ka(HF)= 6.9x10^-4 kb(F-)= 1.4 x 10^-11
Monday, March 1, 2010 at 11:37pm by simi

chemistry
what is the pH of a solution prepared by adding 20.00 mL 0f a 0.10 M acetic acid and 10.00 mL of 0.10 M sodium acetate
Wednesday, October 13, 2010 at 11:04pm by anon

chemistry
1)100ml sample of solution that is 0.2m in both Naf and Hf has 4.0 ml of 1.0m hcl added to it. calculate the ph change of this soultion .ka =7.2*10^-4 2)40 ml of 0.32m benzoic acid if titrated with 60 ml of 0.2 m naoh. clacilate the ph of the resulting solution at the ...
Sunday, March 4, 2012 at 6:28pm by Anonymous

chemsitry
1)100ml sample of solution that is 0.2M in both Naf and Hf has 4.0 ml of 1.0M hcl added to it. calculate the ph change of this soultion .ka =7.2*10^-4 2)40 ml of 0.32M benzoic acid if titrated with 60 ml of 0.2 M naoh. clacilate the ph of the resulting solution at the ...
Sunday, March 4, 2012 at 7:24pm by Anonymous

chemistry
I'm just thinking out loud a little to give you some ideas. If we have an acid, and we know the partition coefficient is moles organic phase/moles aqueous phase, when the solution is pH 10 we should have mostly the salt and K should be small. At pH 2 the acid should be in the ...
Friday, March 12, 2010 at 3:25pm by DrBob222

Chemistry
Which of the following reactions needs to be reversed to solve for the Heat of Neutralization between Hydrochloric Acid and Ammonia? Acetic Acid + Sodium Hydroxide Hydrochloric Acid + Sodium Hydroxide Acetic Acid + Ammonia
Monday, March 29, 2010 at 5:20pm by Cam

chemistry
Which of the following statements about boiling points are true? A. The boiling point of 0.1 m NaF(aq) is lower than the boiling point of 0.1 m methanol(aq). B. The boiling point of a 0.5 m aqueous solution of LiOH is the same as the boiling point of a 0.5 m aqueous solution ...
Thursday, April 18, 2013 at 1:37pm by Anonymous

Chemistry - Buffers
A buffer is formed by adding 500mL of .20 M HC2H3O2 to 500 mL of .10 M NaC2H3O2. What would be the maximum amount of HCl that could be added to this solution without exceeding the capacity of the buffer? A. .01 mol B. .05 mol C. .10 mol D. .15 mol E. .20 mol [I know the ...
Saturday, April 21, 2007 at 2:49pm by alexa

Chemistry
What stoichiometric concentration of the indicated substance is required to obtain an aqueous solution with the pH value shown below? aniline (C6H5NH2) for PH of 9.05 I converted pH to pOH so pOH=4.98 [OH-] =1.122*20^-5 C6H5NH2 + H2O --------> C6H5NH3+ + OH- I: a N/A 0 0 C...
Friday, March 2, 2012 at 8:13pm by Kiana

General Chemistry-Acids/Bases
I'm stuck on a couple of similar problems involving pH and acids/bases 1) What is the final pH of a 1L solution that is initially .15 M HF and .2 M NaF after 10 mL of .02 M HCl has been added? Ka=7.2x10^-4 Do i just calculate the total mols of H and divide by the volume, then ...
Wednesday, November 26, 2008 at 2:18pm by Evelyn

chemistry
An aqueous solution with a pH of 3.00 is diluted from 2.0 L to 4.0 L. Wht is the pH of the diluted solution?
Tuesday, May 5, 2009 at 11:06pm by j

AP Chemistry
(a) What is the pH of a 2.0 molar solution of acetic acid. Ka of acetic acid = 1.8 x 10¯5 (b) A buffer solution is prepared by adding 0.10 liter of 2.0 molar acetic acid solution to 0.1 liter of a 1.0 molar sodium hydroxide solution. Compute the hydrogen ion concentration of ...
Tuesday, February 13, 2007 at 2:55pm by Dave

Chemistry
A solution that contains 2.047 x 10^-1 M of acid, HA, and 1.808 x 10^-1 M of its conjugate base, A-, has a pH of 4.196. What is the pH after 1.629 x 10^-3 mol NaOH is added to 5.961 x 10^-1 L of this solution?
Saturday, January 21, 2012 at 11:17pm by Summer

Chemistry
Calculate the pOH, pH, and percent protonation of solute in the following aqueous solution. 0.059 M quinine, given that the pKa of its conjugate acid is 8.52. Please show me how to do it and not just the answers. Thanks!
Friday, October 29, 2010 at 7:28pm by Alania

chemistry-science
A 500 ml buffer solution contains .2M Acetic acid and .3M sodium acetate. Find the pH of the buffer solution after adding 20 ml of 1M NaOH, what is the pH? (pka = 4.74)
Friday, April 30, 2010 at 3:22am by jess

chem
Consider the titration of 20 mL of .105M Butric Acid HBut, with .125M sodium Hydroxide? calculate the pH before titration calculate the volume of added base to reach the end point calculate the pH halfway to the equivalence point kb(But-)= 6.6x 10^-10 and ka(HBut)= 1.5x 10^-5 ...
Monday, March 1, 2010 at 11:38pm by simi

Chemistry
A 15.5 mL sample of 0.215 M KOH solution requires 21.2 mL of acetic acid in a titration experiment. Calculate the molarity of the acetic acid solution. Please show all steps, I don't understand this.
Monday, May 23, 2011 at 5:51pm by Tina

Inorganic chemistry
A 50 ml sample fo 0.240M NH3(aq) is titrated with aqueous hydrochloric acid. What is the pH after the addition fo 15.0 ml of 0.0600M HCl(aq)? (kb of NH3 = 1.8 x 10^5)
Saturday, April 11, 2009 at 9:35pm by Steve

Chem Problem
I originally asked you the first question and I got the answer 7.7 but theres other parts to the problem but Im not sure what to do In the preparation of a mustard solution, an individual package of mustard was emptied into a beaker and the mass was determined to be 3.809 ...
Wednesday, October 10, 2012 at 12:48am by Kelli

Chem Problem
I originally asked you the first question and I got the answer 7.7 but theres other parts to the problem but Im not sure what to do In the preparation of a mustard solution, an individual package of mustard was emptied into a beaker and the mass was determined to be 3.809 ...
Wednesday, October 10, 2012 at 1:16am by Kelli

chemistry
Joyce, you should have posted your question separately. There is a good chance it will get overlooked by piggy backing on another question. The answer is that acetic acid/sodium acetate mixtures form a buffered solution. The addition of the acetate changes the pH enough that ...
Wednesday, April 29, 2009 at 8:23pm by DrBob222

chemistry
1)Calculate the pH of a 0.10 M NaHX salt solution. Ka (H2X) = 2.1 x 10-2 Ka (HX-) = 4.5 x 10-8 2)Calculate the pH of a 0.10 M NaHX salt solution. Ka (H2X) = 5.3 x 10-5 Ka (HX-) = 5.3 x 10-11
Friday, October 21, 2011 at 8:41pm by yahn

chemistry
Calculate the pH of a 0.10 M NaHX salt solution. Ka (H2X) = 2.1 x 10-2 Ka (HX-) = 7.3 x 10-8 Calculate the pH of a 0.10 M NaHX salt solution. Ka (H2X) = 9 x 10-5 Ka (HX-) = 5.3 x 10-11
Sunday, March 11, 2012 at 6:59pm by Anonymous

chemistry
Pure acetic acid (HC2H3O2) is a liquid and is known as glacial acetic acid. Calculate the ient M 1) Explain why the lattice energy of MgS is approximately 4 times as large as that of NaCl. 2) Draw the Lewis structure for the acetate ion, CH3CO2—, including any important ...
Saturday, July 16, 2011 at 2:01pm by oria

Chemistry
A sample of magnesium metal reacts with hydrochloric acid solution to produce magnsesium chloride solution and hydrogen gas. a)write a balanced chemical equation for this reaction and include phase designations. The phase designations would be s for solid, aq for aqueous, and ...
Thursday, October 7, 2010 at 6:46pm by Anonymous

Chemistry
A sample of magnesium metal reacts with hydrochloric acid solution to produce magnsesium chloride solution and hydrogen gas. a)write a balanced chemical equation for this reaction and include phase designations. The phase designations would be s for solid, aq for aqueous, and ...
Thursday, October 7, 2010 at 8:07pm by Anonymous

Science
Three acids solutions have the following pH: Solution A: pH = 2 Solution B: pH = 5 Solution C: pH = 3 Which solution is made with the acid that has the smallest ionization constant?
Thursday, June 30, 2011 at 11:14pm by Megan

Chemistry
* Fixed Question What is the PH of a buffer made by adding 8.20 grams of sodium acetate(NaCH3CO2) to 500 ml of 0.10 M(molarity) acetic acid(CH3CO2H). Ka for acetic acid is 1.8 x 10^-5.
Sunday, April 14, 2013 at 8:24pm by Lele

chemistry
Calculate the PH concentrated hydrochloric acid if this solution is 24.8% HCL by weight and has a density of 1.16g/ml. I do not understand the right answer 0.90PH Why? Please help My calculation 1.18g/ml x 1000ml x 0.248/36.5 = 7.8M I cannot do?
Sunday, July 29, 2012 at 1:09pm by Fai

Chemistry
CH3COOH + H2O = CH3COO- + H3O+ Acid acetic is a weak acid so not all of it will dissociate. The constant for acid acetic is 1.8 . 10^-5 therefore 1.8x10^-5=(x^2)/(0.2-x) x is the amount that disociated solve the equation and x is 1.88x10^-3 pH=-log(pH)=-log(1.88x10^-3)=2.72
Sunday, January 23, 2011 at 1:38pm by Tom

biology
if a solution has a pH of 4 mix to a solution that has a pH of 9 what will be the pH of the mixed solution? will it be acidic or base? please show me how to calculate it.please i need the answer before tomorrow morning. thank you so much. I had been to other sites but i didn't...
Tuesday, October 20, 2009 at 10:37pm by heather

Chemistry
Consider a 0.80M solution of HCN. The Ka of HCN is 6.2x10-10. What are the major species in solution? Calculate the pH of this solution. ----------------------------------- Ok, so i took a break, came back, and finished the problem. I have an x value of 2.23x10-5. I took the ...
Tuesday, October 18, 2011 at 2:17am by Kevin

Chemistry- Acids and Buffers
Cyanic Acid is a weak acid HOCN + H2O <--> H3O+ +OCN- ka= 3.5*10^-4 a) if 2.5ml of 0.01 M cyanic acid solution is added to 25.0 ml of a formis acid buffer with ph = 3.70, what is the ratio of [OCN-]/[HOCN] in the resulting solution? b) determine the pH of a 0.500 M ...
Monday, April 9, 2012 at 4:21am by Tasneem

chemistry 1046
A.Determine the pH of the solution. a solution that is 1.17% HCl by mass (Assume a density of 1.01 g/mL for the solution.) B. Amphetamine (C9H13N) is a weak base with a pKb of 4.2. Calculate the pH of a solution containing an amphetamine concentration of 279 mg/L.
Tuesday, July 3, 2012 at 8:27am by Anonymous

chemistry
calculate the freezing point and osmotic pressure at 25 degrees celcious of an aqueous solution containing 1.0 g/L of a protein (mm=9.0*10^4g/mol) if the density of the solution is 1.0 g/cm^3
Monday, February 8, 2010 at 9:53pm by heather

College chemistry
Pure acetic acid (HC2H3O2) is a liquid and is known as glacial acetic acid. Calculate the ient M 1) Explain why the lattice energy of MgS is approximately 4 times as large as that of NaCl. 2) Draw the Lewis structure for the acetate ion, CH3CO2—, including any important ...
Friday, July 1, 2011 at 7:59pm by oria

Chem
Please tell me if these are right! What are the [H3O+] and [OH-] for a solution with the following pH values? a. 10.0 I got 1.0*10^-10 for [H3O+] and 1.0*10^-4 for [OH-] b. 5.0 I got 1.0*10^-5 for [H3O+] and 1.0*10^-9 for [OH-] c. 7.00 I got 1.0*10^-7 for [H3O+] and1.0*10^-7 ...
Wednesday, December 8, 2010 at 1:34pm by Jessica

Chemistry
A solution of acetic acid having a concentration of about 0.2M is to be titrated using 0.200M NaOH. Select an indicator for the titration. what salt will the solution contain at the equivalence point? what is the approximate concentration of this salt at the equivalence point...
Saturday, May 15, 2010 at 2:00pm by Alison

Chemistry
3) The pH of a buffer solution made out of 0.20mol/L hydrofluoric acid and 0.30mol/L sodiumfluoride is the same as a buffer solution that is made out of 0.10mol/L of acetic acid and 0.15mol/L of sodium acetate. HF: pH = 3.14 + log(0.3/0.2) = 3.33 HAc: pH = 4.75 + log(0.15/0.1...
Saturday, December 8, 2012 at 2:54pm by DrBob222

chemistry
What molar ratio of acetic acid to sodium acetate is required to create a buffer solution at a pH of 4.89 at 25 degree C? Ka for acetic acid is 1.8 X 10-5 A. 2.9 B.0.56 C.1.4 D.0.72 E.0.2 ( I chose this and got is wrong) I'm lost on how to do these problems, but I started out...
Thursday, March 7, 2013 at 5:35pm by Glen

Chemistry
Which of the following solution has greater density? 1. 100ml of saturated aqueous solution of Lif. (Ksp(Lif)=1.84*10^-3). 2. 100ml of saturated aqueous solution of Hg2F2. (Ksp(Hg2F2)=3*10^-6). (We can assume that adding the dissolved doesn't change the volume of the solution...
Wednesday, July 13, 2011 at 7:22am by qwerty

Chemistry
A beaker with 100 mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 6.10 mL of a 0.260 M HCl solution to the beaker. How much will the pH change? The pKa of acetic ...
Friday, March 18, 2011 at 8:57pm by Sandra

gen chem
a 10 ml vinegar sample was completely neutralized by 22.5 0.2M NaOH solution . calculate the molarity and percent acetic acid in vinegar I keep getting 2.7% acetic acid is this correct? my friend got 27% and if I am wrong where do you think I messed up?
Sunday, November 25, 2012 at 6:16pm by shannan

chemistry
What stoichiometric concentration of the indicated substance is required to obtain an aqueous solution with the pH} value shown below? aniline (C6H5NH2) for PH of 8.90
Sunday, April 11, 2010 at 7:28am by anonymous

chemistry
Select only the True statements about buffer systems. Select all that are True. 1. Starting with NH3(aq) and adding a small amount of HCl(aq) will make a buffered solution. 2. The blood buffer, among other things, is supported by carbonic acid and its conjugate base ...
Friday, March 28, 2014 at 2:45pm by bekah

Chemistry
so i had to calculate the pH of a 100ml solution of .10M acetic acid (ka=1.8x10(-5) I came out to 2.87. But then, they want the pH if 50ml HCL is added. So i thought...Ka = x2/.15M, therefore the square root of .15M x 1.8x10(-5) = .00164(concentration). So -log(.00164) = 2.78...
Thursday, October 20, 2011 at 1:21pm by Kevin

chemistry
19 mL of 0.50 mool/L NaOH which is standardized becomes titrated alongside 24 mL of 0.44 mol/L acetic acid. Determine the pH of the solution Please judge my work: Becasue NaOH and acetic acid react in a 1:1 ratio, initital moles of acetic acid =0.0019 L x 0.44M = 0.000836 mols...
Wednesday, April 9, 2008 at 11:03pm by Joseph

chemistry
The skeletal structures of the two amino acids, glycine and lysine, are given below along with the values of the relevant acid dissociation constants (pKa). (a) For an aqueous solution of glycine alone, calculate the value of pH at which the ratio of the concentration of ...
Saturday, June 1, 2013 at 8:19am by a

Chem
How many milliliters of concentrated hydrochloric acid solution (36.0% HCl by mass, density = 1.18 g/mL) are required to produce 20.0 L of a solution that has a pH of 2.13?
Monday, February 28, 2011 at 1:50am by Anonymous

Chemistry help!!
A chemist wants to be a supercook and wants to create 8%(m/v) acetic acud solution to be "extra strength" vinegar. if pure acetic acid Is a liquid density of 1.049 g/ml. how many ml of acetic acid should be dissolved to male 500 ml of 8% acetic acid? It says to first calculate...
Sunday, April 22, 2012 at 12:42pm by Kate

chemistry
answer is a as acetic acid ionizes only slightly in an aqueous solution
Tuesday, March 23, 2010 at 7:28am by phoebe

Chemistry
Calculate the end point pH, when 25 mL of 0.01 mol/L HCl solution reacts exactly with 25 mL of 0.1 mol/L NH4OH solution. NH3 Kb = 1.8 x 10^-5 This will be the pH of NH4Cl solution. NH4+ + HOH ==> NH3 + H3O^+ Ka = Kw/Kb = (NH3)(H3O^+)/(NH4^+). Solve for H3O^+, then pH = - ...
Thursday, May 31, 2007 at 9:02pm by Raj

Chemistry
Take acetic acid and add NaOH to it. That produces sodium acetate, the base of the acid/base system. To make this work, one needs to use acetic acid and add NaOH but not enough to completely neutralize it. For example, if you took 10 moles acetic acid and added 5 moles NaOH, ...
Tuesday, February 14, 2012 at 5:46pm by DrBob222

chemistry
25 mL of standardized 0.45 mol/L NaOH is titrated with 21 mL of 0.35 mol/L acetic acid. Calculate the pH of the solution
Wednesday, April 9, 2008 at 9:26pm by unknown

Chemistry
Given that the pKa for Acetic Acid is 4.77, calculate the expected pH of the buffer solutions using the Henderson-Hasselbalch equation and the concentrations of Acetic Acid and Acetate added to the 250 ml Erlenmeyer flask
Friday, March 18, 2011 at 8:10pm by M_Joe

Chemistry
Chester makes 1L of a 0.01M HCl solution and measure the pH. Burt then adds 5.80 g of sodium chloride to Chester’s solution and measures the pH. Calculate the difference between the two pH values obtained.
Friday, February 14, 2014 at 6:05pm by Anonymous

chemistry
When 5.00 g of barium hydroxide are added to 250.0 mL of 0.250 hydrochloric acid in a calorimeter, the temperature off the solution increases from 25.0 C to 28.0 C. Calculate the enthalpy ( in kJ per mole of water) given the density of the hydrochloric acid is 1.01 g/mL and ...
Saturday, June 1, 2013 at 2:16am by Jen

chem
reposted again a 275mL sample of vapor in equilibrium with 1-propylamine at 25C is removed and dissolved in 0.500L of H20. For 1-propalamine, Kb=3.72*10^-4 and the vapor pressure at 25C is 215 torr. (a)What should be the pH of the aqueous solution? (b) How many mg of NaOH ...
Tuesday, March 22, 2011 at 8:44pm by kate-------------------------------------

Chemistry -- to Dr.Bob
No, because sodium acetate is the salt of a strong base and a WEAK acid, (as opposed to HCl which is a strong acid) so you just follow the steps I did. write the equation. You have mols NaOH You have mols acetic acid. So how much sodium acetate (the salt) is produced? What is ...
Friday, May 2, 2008 at 9:41pm by DrBob222

chemistry
why does the pH of an aqueous solution change after HCl solution has been added
Tuesday, June 15, 2010 at 9:21pm by meredith

General Chemistry 1412 pH question
Calculate the pH of 500 mL of 0.200 M acetic acid, CH3COOH, to which 0.0750 mol of sodium acetate,NaCH3COO, has been added.
Wednesday, April 18, 2012 at 9:33pm by jennyfier

chemistry
a 205 mg sample of diprotic acid is dissolved in enough water to make 250 ml of solution. The pH of this solution is 2.15. A saturated solution of calcium hyrdoxide (Ksp=1.3*10^-6) is prepared by adding excess calcium hydroxide to water and then removing the undissovled solid ...
Sunday, March 4, 2012 at 8:09pm by cat

Chemistry
Here's what I did: So I set values for: [Acetic Acid] = y [H3O+] = 10^-5 [Acetate] = 0.1M - y Ka = 10^-4.76 And from the equation: Ka = [Acetate][H3O+]/[Acetic Acid], I found y, or the molarity of acetic acid, to be 10^-6/(10^-5 + 10^-7.46). And from this, I also got the ...
Friday, March 18, 2011 at 8:57pm by Sandra

chemistry
A 2.5 g sample of NaOH (Mw = 40.00) was dissolved in water to give a solution of final volume 250 cm3. (i) With reasons, state whether NaOH is a strong or a weak base. Give the conjugate acid of NaOH and decide whether this conjugate acid is acid, alkaline or neutral. (ii) ...
Sunday, April 21, 2013 at 10:01am by LUx

General Chemistry
How do I calculate the ratio of weak base to weak acid in a methyl amine buffer solution at pH=10.645 and pH=11.645 and pH=9.645?
Monday, February 27, 2012 at 8:05pm by Nhi Song

Molality
An aqueous solution contains 8.7% NaCl by mass. 1. Calculate the molality of the solution. 2. Calculate the mole fraction of the solution.
Saturday, January 30, 2010 at 5:25pm by Kyle

Chemistry
The pH of a solution is 11.30. In order to find the concentration of H+, wouldn't I simply take the pH of the solution and plug it into the formula 10^-pH?
Wednesday, September 16, 2009 at 11:21pm by Anonymous

Chem I
Ok here is another one! Concentrated aqueous HClO4 has a concentration of 14.8 M. Calculate the concentrations of ALL ions present in a solution prepared by pipetting 5.00mL of concentrated HClO4 into a 1000.0-mL volumetric flask and filling to the mark. Also calculate the pH ...
Monday, November 15, 2010 at 10:17pm by Natalea

Chemistry
Calculate the pH at the equivalence point of 25.0 mL of a 0.100 M acetic acid, CH3COOH, titrated with a 0.100 M sodium hydroxide, NaOH. Ka of acetic acid is 1x10^-5
Sunday, April 11, 2010 at 12:53pm by Anonymous

chemistry
MF16032: What is the percent dissociation of acetic acid if the solution has pH = 4.74 and pKa = 4.74? is it 50% yes, 50%. Do you know how to prove that? Did you calculate it or did you make an educated guess?
Tuesday, May 1, 2007 at 12:54am by joe

Chemistry
If 20ml of glacial acetic acid (pure HC2H3O2) is diluted to 1.5L with water, what is the pH of the resulting solution. The density of glacial acetic acid is 1.08g/ml
Monday, August 2, 2010 at 9:37pm by Kristen

College Chemistry
What is the pH when 10 mL of 1 M acetic acid is added to pure water so that the final volume is 100 mL? The Ka for acetic acid is 1.74 x 10^(-5)
Friday, September 23, 2011 at 10:37pm by Jamal

chemistry
I assume you meant acetic acid (and not acidic acid). Also, I assume you mean to add M so that the sentence reads .....1000 mL of a 0.10 M buffer (I have added M). Use the Henderson-Hasselbalch equation. pH = pKa + log [(base)/{acid)] pKa = 4.74 for acetic acid. You want pH = ...
Tuesday, April 20, 2010 at 8:30pm by DrBob222

chemistry 1st year, for midterm help
Hi, Can any1 help with theses questions. I need to solve these because there will be similar questions on the midterm for me, coming week. Btw I have tried few. 1. How many milliliters of a 15.0%, by mass solution of KOH (Aq) ( d= 1.14g/mL ) are required to produce 27.0 of a ...
Wednesday, February 11, 2009 at 11:10pm by ur class fella

Chemistry
Consider a 0.80M solution of HCN. The Ka of HCN is 6.2x10-10. What are the major species in solution? Calculate the pH of this solution.
Tuesday, October 18, 2011 at 1:15am by Kevin

Physical Chemistry HELP!!!!!
A solution of the sugar mannitol ( molar mass 182.2 g/mol ) is prepared by adding 54.66 g of mannitol to 1.000 kg of water. The vapor pressure of pure liquid water is 17.54 torr at 20o C. Mannitol is nonvolatile and does not ionize in aqueous solution. a.) Assuming that ...
Saturday, October 14, 2006 at 5:29am by Lan

Chemistry
This is for a titration, to measure the amount of acid that can be neutralised by gaviscon. I know how to work out the first 3 but I'm not sure on the others. I think i need to use the calculation c=n x v but i don't know where and why? Theory. How do you work them out? (i)...
Tuesday, December 9, 2008 at 5:19pm by Anonymous

Chemistry
If 15.omL of 0.0250 M aqueous H2SO4 is required to neutralize 10.0 mL of aqueous solution of KOH, what is the molarity of the KOH solution?
Monday, May 23, 2011 at 11:03am by Tina

Chemistry
Identify the solvent and the solute in vinegar, a dilute aqueous solution of acetic acid.
Tuesday, April 13, 2010 at 6:12pm by Danny

Chemistry
Identify the solvent and the solute in vinegar, a dilute aqueous solution of acetic acid.
Tuesday, April 13, 2010 at 8:27pm by Danny

Chemistry
If 31.00 mL of a dilute solution of lime water (calcium hydroxide) required 10.10 mL of 0.246 M hydrochloric acid solution for neutralization to a methyl red end point, calculate the molarity of the lime water. Can you please explain how to do it? Do I use M1V1=M2V2?
Saturday, April 2, 2011 at 3:22pm by Lara

Chemistry
The Ka of hydrazoic acid (HN3) is 1.9 × 10-5 at 25°C. What is the pH of a 0.35-M aqueous solution of HN3?
Thursday, December 10, 2009 at 11:06pm by Ericka

chemistry
for a .001M solution of methionine: a) calculate the isoelectric pH b) calculate the isoionic pH
Sunday, April 7, 2013 at 7:58pm by Lana

chemistry
A saturated aqueous solution of calcium hydroxide has a pH of 12.25. What is the [Ca2+] of such a solution?
Tuesday, March 18, 2008 at 11:06pm by Anonymous

chemistry
a 1.00 L aqueous solution contained 5.80 g of NaOH. what is the pH of the solution? Can someone help me out with the setup of this?
Wednesday, April 28, 2010 at 4:13pm by Anna

Chemistry
what is the pH of a 0.025 M aqueous solution of sodium propionate, NaC3H5O2? What is the concentration of propionic acid in the solution?
Monday, August 8, 2011 at 7:57pm by Henry

Chemistry
A saturated aqueous solution of calcium hydroxide has a pH of 12.25. What is the [Ca 2+] of such a solution?
Saturday, April 14, 2012 at 9:41pm by Andy

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